Calculate the density of oxygen, , under each of the following conditions:
STP
1.00atm and 25.0 degrees celsius
Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.
PV = nRT
Since n = mols = g/molar mass (molar mass = MM), then we can substitute g/MM for n.
PV = (g/MM)RT
Then rearrange as
P*MM = (g/V)*RT
where g/V is g/L or the density.
Just substitute the numbers to get your answers. Post your work if you get stuck.
1.56
1.46,1.98
To calculate the density of oxygen at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
STP conditions are defined as a pressure of 1 atmosphere and a temperature of 0 degrees Celsius (273.15 Kelvin).
First, let's convert the temperature of 25.0 degrees Celsius to Kelvin:
T = 25.0 + 273.15 = 298.15 K
Now, we'll substitute the values into the ideal gas law equation, assuming 1 mole of gas (oxygen in this case) to make the calculations easier:
(1.00 atm) * (V) = (1 mol) * (0.0821 L*atm/mol*K) * (298.15 K)
Solving for V (volume):
V = (0.0821 L*atm/mol*K * 298.15 K) / (1.00 atm)
V = 24.465 L
Now that we have the volume, we can calculate the density by dividing the mass of oxygen by the volume.
The molar mass of oxygen (O2) is approximately 32 grams/mol. The molecular formula for oxygen is O2 because it exists as a diatomic molecule.
To convert grams per mole to grams per liter, we can divide by the molar volume of oxygen at STP, which is 22.4 L/mol.
Density = (32 g/mol) / (22.4 L/mol)
Density = 1.43 g/L
So, the density of oxygen at STP is 1.43 grams per liter.